By Alec “Dr. Bathroom” Levy Niteesh “The Yellow Dart” Chitturu

NomenclatureCation-Electron-deficient atom/molecule (+

charge)Atoms in transition metals, alkalines, alkaline

earths typically form cationsEx.: Ca2+ Fe2+ Li+

Transition metals include Roman Numerals except Zn2+ Ni2+ Ag+

Anion-Electron-surplus atom/molecule (- chargeForm in halogens, chalcogens, pnictogens, and

polyatomic moleculesEx: F- O2- N3- SO2-

NomenclatureAtom-smallest unit of element that retains its

properties, includes mono- and poly-Compound-2 different elements bonded

togetherMolecule-Covalently bonded atomsSalt-Combination of 2 or more ions bonding

to form a neutral compoundSame thing as a neutral ionic compound,

which consists of a metal cation and nonmetal anion

Acid NomenclatureAcids-Contains H+ cation-ide hydro_____ic acid-ate _____ic acid-ite ______ous acidEx: Sulfide=hyrdosulfuric acidEx: Sulfate=sulfuric acidEx: Sulfite=sulfurous acid

Bonding & FormulasCovalent compounds-2 or more nonmetals,

come first in formula, except for F and OOrganic compounds-Hydrocarbons, consists

of only C and HAlkanes-Carbon backbone, fills in excess with

H, ends with –ane 1=meth 2=eth 3=prop 4=but 5+=binary

Alcohols-Adds O to chain, ends in -anol

Common Anions1- H- (Hydride ion), F- (Fluoride ion), Cl-

(Chloride Ion), Br- (Bromide ion), I- (Iodide ion), CN- (Cyanide ion), OH- ( Hydroxide ion), C2H3O2

- (Acetate ion), ClO3

- (Chlorate ion) ClO4-

(Perchlorate ion), NO3- (Nitrate ion), MnO4

- (Permanganate ion)

2- O2- (Oxide ion), O22- (Peroxide ion), S2- (Sulfide

ion), CO32- (Carbonate ion), CrO4

2- (Chromate ion), Cr2O7

2- (Dichromate ion), SO42- (Sulfate ion)

3- N3- (Nitride ion), PO43- (Phosphate ion)

Atomic StructuresAngstrom-Å=10-10 meters=size of an atomProton-Subatomic particle with positive

charge of 1, in the nucleusNeutron-Subatomic particle with neutral

charge, in the nucleusElectron-Subatomic particle with negative

charge of 1, in energy orbitalsProtons and Neutrons consist of 99.99% of

mass1 electron=1/1800 proton

Isotopic Notation

Isotopes have same number of protons but different number of neutrons and are chemically identical

A-Mass number=protons+neutronsq-Charge=electron+protonsZ-Atomic number=protons

XA

Z

q

Isotopic Abundance/Molar MassTo calculate isotopic abundance from molar

massEx: Average mass of sample is 1.614 g/mol.

Molar mass of hydrogen-1 is 1.00782, molar mass of deuterium is 2.01410. What is the abundance of the two isotopes?

Answer: hydrogen-1=39.76%, deuterium=60.24%

Balancing reaction equationsGiven: C24H46O3 + O2CO2 + H2O

Answer : C24H46O3 + 34O224CO2 + 23H2O

It’s 1.5-glyceride

Isn’t Chemistry pHun?

Mass-mole relationship1 mole of a substance is equal to 6.022 x 1023

particle1 mole of substance is equal to its amu but in

gramsPoly-atomic substances moles are a sum of its

constituentsEx: C24H46O3 has 24 C, 46 H, and 3 O. Thus:

(12.0107 x 24) + (1.00794 x 46) + (15.9994 x 3)=382.62024

g/mol

Empirical formulas/percent compositionGiven percent composition by mass

spectrometry, the empirical formula of a molecule is what?

54.50% carbon, 13.72% hydrogen, 31.78% nitrogen

Assume given values are in grams, then calculate for moles

Divide moles by lowest value of molesAnswer is subscript of empirical formulaTo determine molecular formula, molar mass

must be known Ex: 88.15 g/mol

Limiting/Excess ReactantsTo determine limiting reactant, balance

equation and solve for both reactantsLower value is limiting, the higher one is

excess

Percent YieldPercent Yield=(actual or experimental

value)/(theoretical values determined by limiting reactant)

Easy? Yes/No?

IT’S A GAS GAS GAS!!!Qualitative: pressure, volume, number of moles, and

temperature are at work, along with R, the gas constant

Boyle’s Law: Volume of gas at constant temperature is inversely proportional to pressure V=k ∙ 1/p

Charles’s Law: Volume of gas at constant pressure is directly proportional to absolute temperature V=k ∙ T

Avogadro’s Law: Equal volumes of gases at equal temperature and pressure contains equal number of molecules, and volume of gas at constant pressure and temperature is directly proportional to number of moles V=k ∙ n

Ideal Gas LawPV=nRTR is the ideal gas constant, equal to 0.08206

L-atm/mol-KVolume of a gas at STP is 22.41 LTo calculate density, calculate concentration

(mol/L) and convert to g/cm3 (1 mL=1 cm3)

PV=nRT in action…Given: pressure is 1020 torr, volume is 1.5 L,

and temperature 37. 4 degrees Celsius, mass of sample is 2.530 g, what is the molar mass?

1020 torr=1.342 atm37.4 degrees Celsius=310.55 degrees Kelvinn=PV/RT=.07899 molMolar mass=g/mol=2.530 g/ .07899 mol=

32.03 g/molIt’s O2!

Partial PressureDalton’s law of partial pressures: Total

pressure of a mixture of gases equals the sum of the pressures that each would exert alone

Applies only for ideal gases!!!Pt = P1 + P2 + P3 …. + Pn

Mole fraction (X)=Moles of given gas/Total Moles of gas

Pn = Xn Pt

Kinetic Molecular TheoryGases consist of large amounts of molecules in

continuous random motionThe molecules have negligible volume compared

to the total volume the gas occupiesThere are negligible attractive or repulsive forces

between those moleculesThe average kinetic energy of the molecules

remains constant (the collisions are perfectly elastic)

The molecule’s average kinetic energy is proportional to the absolute temperature

Root Means Square SpeedVelocity=u=√(3RT/M)R=gas constantT=absolute temperatureM=kg/molLighter molecules move on average faster

than heavier molecules

Graham’s rates of effusion/diffusionEffusion: Gas escaping into a vacuumDiffusion: Gas mixing into another gas, going

from high concentration to low concentrationRate A escapes/Rate B escapes= ua/ub =

√Mb/Ma

Van der Waals’s equationReal (non-ideal) gas equationMolecules DO occupy space, thus takes up volumeMolecules DO sometimes attract each otherCorrection factors are needed(Preal + a(n/v)2)(Vcontainer – bn)=nRTa=attractive coefficient, expressed in atm ∙ L2/mol2

b=volume coefficient, expressed in L/mol

(Das Good?)

Fin

Dr. Bathroom and the Yellow Dart…Away!?!